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18 Nov 2019
In a 0.55 M solution, a weak acid is 3.4% dissociated. Calculate the [H_3O^+], pH, [OH^-], and pOH of the solution. [H_3O^+] = M [OH^-] = times 10 M pH = pOH = calculate K_a of the acid. K_a =
In a 0.55 M solution, a weak acid is 3.4% dissociated. Calculate the [H_3O^+], pH, [OH^-], and pOH of the solution. [H_3O^+] = M [OH^-] = times 10 M pH = pOH = calculate K_a of the acid. K_a =
Bunny GreenfelderLv2
30 Jul 2019